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complex formation equilibria with Ag+ for EDTA, CN-, NH3, I-
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- The accompanying data (1.00-cm cells) were obtained for the spectrophotometric titration 10.00 mL of Pd(II) with 2.44 10-4 M Nitroso R(O. W Rollins and M. M. Oldham, Anal. chem .,1971, 43, 262, DOI: 10.1021/ac60297a026). Calculate the concentration of the Pd(II) solution, given that the ligand-to-cation ratio in the colored product is 2:1Why is EDTA complex formation less complete at lower pH?Using VBT, predict the geometry of the tetraaminocadmium(II) complex ion.
- A second calibration standard solution of an iron(III) salicylate complex was prepared in two steps. First, 12.9 mL of a 0.481 M stock solution was diluted with solvent to make 100.0 mL of the first calibration standard solution and, secondly, 86.6 mL of that first calibration solution was diluted to 100 mL to make the second calibration standard. What is the molar concentration of the second calibration standard solution? Report your answer to 3 significant figures.The concentration of iron in a solution can be determined using UV?Vis spectrophotometry by reacting the iron with 1.10-phenanthroline to produce a colored complex. The following data were obtained for a series of standard solutions of iron/1,10-phenanthroline complex measured in a 1.00 cm cell. Concentration (M) Absorption 0.50x10-4 0.109 1.0x10-4 0.218 2.0x10-4 0.436 3.0x10-4 0.656 4.0x10-4 0.872 a.Prepare a Beer’s law plot using the above data b.Calculate the concentration of an iron 1, 10-phenanthroline complex solution that has an absorbance of 0.317 c.Calculate the molar absorptivity of the iron/1, 10-phenanthroline complexA second calibration standard solution of an iron(III) salicylate complex was prepared in two steps. First, 10.0 mL of a 0.100 M stock solution was added to 90.0 mL of solvent to make 100.0 mL of the first calibration standard solution and, secondly, 80 mL of that first calibration solution plus 20.0 mL of solvent were mixed to make the second calibration standard. What is the concentration of the second calibration standard solution?
- Janine's research focuses on the ability of quercetin, a flavonoid and natural dye, to detect the presence of Co2+ in wastewater samples. She prepared a set of calibration standard solutions by adding an excess of quercetin to solutions of varying Co2+ concentration and maintaining it at pH 6.4 using a Tris-HCl buffer. The reaction yields a colored complex solution that has a maximum absorbance at 440 nm:Co2+ + 2 Quercetin --> Co(Quercetin)22+ The absorbance measurements for the calibration solutions prepared are shown in the tables; a cuvette with a 2.50 cm path length was used. [Co2+], in M Absorbance Color Wavelength range (nm) 0.05 0.100 Red 625-740 0.10 0.166 Orange 590-625 0.20 0.285 Yellow 565-590 0.30 0.367 Green 490-565 0.40 0.454 Blue 440-490 0.50 0.571 Violet 380-440 Part of her research is to determine the extent of Co2+ pollution in a stream near a pharmaceutical company. She obtained a 50.0-mL sample of the stream water and buffered it to pH 6.4. She…Calculate the conditional formation constant (K'' NiY) of the [NiY]2- complex in 0.050 M NH3 and 0.090 M NH4Cl buffer solution. The formation constants of nickel amine complexes are respectively K1 = 102.75, K2 = 102.20, K3 = 101.69, K4 = 101.15, K5 = 100.71, K6 = 10-0.01. (KNiY = 4.2x1018, KNH3 = 1.74x10-5)What is the ligand to metal ratio for SCN-1 and Fe+3?
- Draw structures for the following complexes: fac-triaquacyanidodinitrito-kN-chromate(III) ion di-m-oxidobis(tetramminecobalt(III)) iona. write the net ionic equation involved in the formation of copper complexes in: Reagent added ligand added 1 control - 2 0.5 mL of 12M NH3 NH3 3 5 drops of 5M HCl Cl- b. starting from the copper (ii) complexes in the table above, write the net ionic equation involved in the ligand substitution reactions as observed in: Reagent added reagent added 1a 0.25 mL of 12 MNH3 1b 0.22g of KCl 2a 0.25 mL H2O 2b 0.22g of KCl 3a 0.25 mL H2O 3b 0.25 mL of 12M NH3A cyanide solution with a volume of 13.72 mL was treated with 25.00 mL of Ni2+ solution(which contained an excess of Ni(II) ions) to convert the cyanide to the complex ion tetracyanonickelate(II): 4CN- + Ni2+ → 6 Ni(CN)2- The excess Ni 2+ was then titrated with 10.15 mL of 0.01307 M EDTA. One mole of this reagent reacts with one mole of Ni(II) as follows: Ni(CN)42- does not react with EDTA. If 39.35 mL of EDTA was required to react with 30.10 mL of the original Ni 2+ solution, calculate the molarity of CN- in the 13.72 mL cyanide sample.